Answer:
1. Q = 8.66 KJ
2. Q = 7.58 Kcal
3. Q = 0.71 KJ
4. Q = 24.31 Kcal
Explanation:
1. The quantity of heat absorbed can be determined by:
Q = mcΔθ
where: Q is the quantity of heat absorbed or released, m is the mass of the substance, c is the specific heat capacity of water = 4.2 j/g and Δθ is the change in temperature.
= 45.2 × 4.2 × (76.9 - 31.3)
= 8656.704
∴ Q = 8.66 KJ
The quantity of heat absorbed is 8.66 KJ.
2. Q = mcΔθ + mL
Where L is the latent heat of fusion of ice = 334 J.
= m(cΔθ + L)
= 72.1(4.2 × 25.2 + 334)
Q = 31712.464 J
= 7579.466 calories
The total heat released is 7.58 Kcal.
3. Q = mcΔθ
= 55.5 × 0.129 × (123.4 - 24.6)
= 707.3586
The quantity of heat required to increase the temperature of gold is 0.71 KJ.
4. Q = mL
Where: L is the specific latent heat of vaporization = 533 calories.
Q = 45.6 × 533
= 24304.8
The quantity of heat required to change water to steam is 24.31 Kcal.
Answer:
3.72
Explanation:
Given data:
Mass of object = 82.2 g
Volume of water = 25.0 mL
Volume of water + object = 47.1 mL
Density of object = ?
Solution:
Volume of object:
Volume of object = (Volume of water + object) - Volume of water
Volume of object = 47.1 mL - 25.0 mL
Volume of object = 22.1 mL
Density of object:
d = 82.2 g/ 22.1 mL
d = 3.72 g/mL
5.57 × 10²⁵ molecules of Br₂ will have a mass of 14862.33g
HOW TO CALCULATE MASS:
- The mass of an element can be calculated by multiplying the number of moles by its molar mass. That is;
mass (g) = moles (mol) × molar mass (g/mol)
- However, the number of moles in 5.57 × 10²⁵ molecules of Br₂ will be calculated first by dividing the number of molecules by Avogadro's number.
no. of moles = 5.57 × 10²⁵ ÷ 6.02 × 10²³
no. of moles = 5.57/6.02 × 10²⁵-²³
no. of moles = 0.93 × 10²
no of moles = 93 moles
Molar mass of Br₂ = 159.81g/mol
Mass of Br₂ = 93 × 159.81
Mass of Br₂ = 14862.33g
- Therefore, 5.57 × 10²⁵ molecules of Br₂ will have a mass of 14862.33g.
Learn more: brainly.com/question/10384503?referrer=searchResults
ANSWER:
D = M/V
6.0/12.0 = 0.5
0.5 is your answer
~aliens wife dun dun dun....
1. 254 cal = 1,062.736 joules
2. 126 cal = 527.184 joules
3. 98 cal = 410.032 joules
4. 704 cal = 2,945.536 joules
5. 682 cal = 2,853.488 joules